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Why Real gases do not obey gas laws?
Real gases do not obey gas laws because these gases contains forces of attractions among the molecules..and the gases which do not contain forces of attraction among their molecules are called ideal gases and they obey gas laws.
Which gas is least likely to obey the ideal gas laws at very high temperatures and very low temperatures A. Kr B. Ne C. He D. Xe Why?
Gas D. Xe (Xenon) is least likely to obey the ideal gas laws at very high and very low temperatures. This is because Xenon has a larger atomic size and heavier mass compared to the other gases listed, making it more likely to exhibit non-ideal gas behavior due to intermolecular forces and molecular interactions becoming more significant at extreme conditions.
Why Gay-Lussac laws are only applicable in gases?
Gay-Lussac's laws specifically deal with the relationship between pressure and temperature in a gas, and they are based on the assumption that gas particles are in constant motion and collide with each other and the walls of their container. This assumption is not valid for liquids or solids, where the particles are closely packed and do not move as freely as gas particles. Therefore, these laws are only applicable to gases.
Would a gas whose molecules were true geometric points obey the ideal gas law?
If gas molecules were true geometric points (ie had zero volume) AND had zero intermolecular interaction (such as attraction or repulsion), then the gas would obey the ideal gas law. Gases composed of small, non-interactive molecules (such as helium gas) obey the ideal gas law pretty well (as long as the gas is low density and temperature is rather high). For non-ideal gases, at least two correction factors are often used to modify the ideal gas law (correcting for non-zero volume of gas molecule and intermolecular attraction) such as in the Van der Waals equation for a real gas.
When is an ideal gas an imaginary gas?
An ideal gas is never an imaginary gas; it is a theoretical concept used to describe the behavior of real gases under certain ideal conditions, such as negligible volume of gas particles and no intermolecular forces. It is an approximation that helps simplify the study of gas behavior.
What is the imaginary gas that perfectly fits all the postulates of the kinetic molecular theory?
ideal gas
Why Real gases do not obey gas laws?
Real gases do not obey gas laws because these gases contains forces of attractions among the molecules..and the gases which do not contain forces of attraction among their molecules are called ideal gases and they obey gas laws.
A gas that follows the kinetic molecular theory and gas laws exactly is known as a?
An ideal gas. Ideal gases are theoretical gases that perfectly follow the assumptions of the kinetic molecular theory and gas laws, such as having particles that are point masses and exhibit perfectly elastic collisions.
The temp at which real gases obey the ideal gas laws over a wide range of pressure what is this temp known as?
boyles temprature
What gas conforms to the gas laws at all conditions of temperature and pressure?
An ideal gas conforming to the ideal gas law (PV = nRT) would behave at all conditions of temperature and pressure. However, in reality, no gas perfectly conforms to the gas laws under all conditions.
Which gas is least likely to obey the ideal gas laws at very high temperatures and very low temperatures A. Kr B. Ne C. He D. Xe Why?
Gas D. Xe (Xenon) is least likely to obey the ideal gas laws at very high and very low temperatures. This is because Xenon has a larger atomic size and heavier mass compared to the other gases listed, making it more likely to exhibit non-ideal gas behavior due to intermolecular forces and molecular interactions becoming more significant at extreme conditions.
What is an imaginary gas that conforms perfectly to the kinetic molecular theory callled?
That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.
How do you use word disabling in sentence?
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Why Gay-Lussac laws are only applicable in gases?
Gay-Lussac's laws specifically deal with the relationship between pressure and temperature in a gas, and they are based on the assumption that gas particles are in constant motion and collide with each other and the walls of their container. This assumption is not valid for liquids or solids, where the particles are closely packed and do not move as freely as gas particles. Therefore, these laws are only applicable to gases.
All collisions between gas particles are considered to be perfectly what?
All collisions between gas particles are considered to be perfectly elastic, meaning there is no loss of kinetic energy during the collision. This assumption allows for the conservation of momentum and energy to be applied to gas particle interactions.
Do ideal gases have volume and intermolecular attractive forces?
Ideal gases are considered to have no volume and no intermolecular attractive forces. This assumption allows for simplified mathematical relationships in gas laws. In reality, no gas perfectly fits the ideal gas model, but ideal gases are a useful theoretical concept for understanding gas behavior.
Why can an ideal gas not be liquefied?
An ideal gas is not a real thing, just an idea. The definition of an ideal gas is one where there are no forces between the particles. If there are no forces, there is nothing to bring the particles together into a liquid. In a real gas of course there are forces of attraction which keep the particles together when they are moving sufficiently slowly.
